Question

1. Write a balance ionic equation to represent the oxidation of iodide (I-) by permanganate ion (MnO4-) in basic solution to yield molecular iodine (I2) and manganese (IV) oxide (MnO2). 2. Balance the following equation for the reaction in an acidic medium by the half reaction method: Fe2+ + MnO4- -> Fe3+ + Mn2+

          1. Write a balance ionic equation to represent the oxidation of iodide (I-) by permanganate ion (MnO4-) in basic solution to yield molecular iodine (I2) and manganese (IV) oxide (MnO2).
2. Balance the following equation for the reaction in an acidic medium by the half reaction method:
Fe2+ + MnO4- -> Fe3+ + Mn2+

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1. Write a balance ionic equation to represent the oxidation of iodide (I-) by permanganate ion (MnO4-) in basic solution to yield molecular iodine (I2) and manganese (IV) oxide (MnO2).
2. Balance the following equation for the reaction in an acidic medium by the half reaction method:
Fe2+ + MnO4- -> Fe3+ + Mn2+

Added by Jorge L.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Madhur L

12/05/2022

Step 1

** The balanced ionic equation is: \[6I^- + 2MnO_4^- + 4H_2O \rightarrow 2MnO_2 + 3I_2 + 8OH^-\] ** Show more…

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Write balanced ionic equation to represent the oxidation of iodide (I-) by permanganate ion (MnO4-) in basic solution to yield molecular iodine (I2) and manganese (IV) oxide (MnO2). Balance the following equation for the reaction in an acidic medium by the half reaction method: Fe2+ + MnO4- -> Fe3+ + Mn2+

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Transcript

00:01 Hi, in this question we are asked to write the balanced ionic equation in basic medium that represents the oxidation of iodide ion by the permagnate ion which yields the molecular iodine and magnesium 4 oxide.

00:16 We can write the balanced ionic equation as 6 i minus plus 2 mno 4 minus plus 4 h2 gives 2.

00:30 Mn o2 plus 3i2 plus 8 oh minus.

00:38 This is the balance ionic equation in basic medium.

00:42 In second part of the question we are given with the reaction, fe2 plus plus mno4 minus gives fe3 plus plus mn2 plus.

00:50 We are asked to balance this equation in acidic medium by half reaction method.

00:56 Here we can see that fe is present in plus 2 oxidation state and in product side it is present in plus 3 oxidation state.

01:05 In mn of 4 minus, magnesium is having plus 7 oxidation state towards the reactant side and in product side it has plus 2 oxidation state.

01:14 We can see there is decrease in oxidation state in case of mn.

01:20 Therefore we can say it is the reduction and in case of fe from pretextion.

01:28 Plus 2 it is converted into plus 3, therefore it is the oxidation.

01:35 We can write the oxidation half reaction and reduction half reaction in this manner.

01:40 The first step to balance the reaction is to balance the atoms other than oxygen and hydrogen.

01:47 In oxidation half reaction we can say the fe atom is balanced and in reduction half we can say mn is also balanced.

01:55 Therefore, we have to proceed to next step...

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